Search found 61 matches
- Tue Dec 08, 2020 7:53 am
- Forum: Bronsted Acids & Bases
- Topic: Textbook Fundamentals J.7
- Replies: 2
- Views: 349
Re: Textbook Fundamentals J.7
Hi! Zinc ion is usually 2+ charged because its electron configuration is [Ar]3d 10 4s 2 , so it readily loses 2 valence electrons in 4s-orbital, similar to Group 2 metals. Then, since hydroxide ion and nitrite ion are both 1- charged, the "zinc:anion" ratio is 1:2. This gives you Zn(OH) 2 ...
- Tue Dec 08, 2020 1:21 am
- Forum: Acidity & Basicity Constants and The Conjugate Seesaw
- Topic: Ka
- Replies: 1
- Views: 130
Re: Ka
In my understanding, K a is only dependent on the type of acid, while pH is dependent on both the type of substance and the concentration of the solution as well. K a tells you the extent to which an acid dissociates into H+ and A-. ( K_a = \frac{[H^+][A^-]}{[HA]} ) Strong acids almost completely di...
- Tue Dec 08, 2020 1:02 am
- Forum: Calculating pH or pOH for Strong & Weak Acids & Bases
- Topic: 6B #1
- Replies: 1
- Views: 93
Re: 6B #1
Hi! Suppose the initial molar concentration of HCl is x (mol/L), then the final concentration is 0.12x (mol/L). Because HCl is a strong acid, we assume that it completely dissociates into H+ and Cl- in the solution. Therefore: - In the initial solution, [H+] initial =[Cl-] initial =x (mol/L); - In t...
- Tue Dec 08, 2020 12:49 am
- Forum: Amphoteric Compounds
- Topic: Amphoteric: acid and/or base
- Replies: 4
- Views: 516
Re: Amphoteric: acid and/or base
Hi! In the Bronsted-Lowry definition, an acid is a proton donor and a base is a proton acceptor. In the Lewis definition, an acid is a electron acceptor and a base is an electron donor. (The Lewis definition has a wider range of application than Bronsted, but in many cases the Bronsted definition is...
- Tue Dec 08, 2020 12:07 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Textbook 2E #9
- Replies: 1
- Views: 113
Re: Textbook 2E #9
Hi! The question asks us to draw ICl3 Here's a screenshot of my textbook.
- Tue Dec 01, 2020 9:35 am
- Forum: Naming
- Topic: Charge (oxidation state) of atoms/molecules
- Replies: 6
- Views: 295
Re: Charge (oxidation state) of atoms/molecules
Hi! Here are the general guidelines for finding oxidation states: https://www.chemguide.co.uk/inorganic/r ... tates.html
The oxidation state of a ligand is equal to its charge; and the sum of oxidation states in a coordination compound is equal to its overall charge. Hope it helps!
The oxidation state of a ligand is equal to its charge; and the sum of oxidation states in a coordination compound is equal to its overall charge. Hope it helps!
- Tue Dec 01, 2020 12:54 am
- Forum: Shape, Structure, Coordination Number, Ligands
- Topic: Qualifications for Polydentate
- Replies: 3
- Views: 227
Re: Qualifications for Polydentate
Hi! Like what the previous answer says, sigma bonds can rotate while the existence of pi bonds restrict rotation. So a ligand (with several lone pair sites) that consists of all single bonds can probably "get around" and form multiple bonds at the same time. Also, there should be enough sp...
- Tue Dec 01, 2020 12:45 am
- Forum: Naming
- Topic: Order of Molecules
- Replies: 6
- Views: 376
Re: Order of Molecules
Hi! In the lecture Dr. Lavelle gave an example [Co(NH3)5Cl], where NH3 is placed before Cl. So I guess the order of the ligands doesn't really matter, as long as the TM cation is the first one it should be fine!
- Tue Dec 01, 2020 12:24 am
- Forum: Shape, Structure, Coordination Number, Ligands
- Topic: Questions About Textbook Problem 9C.5
- Replies: 1
- Views: 128
Re: Questions About Textbook Problem 9C.5
Hi! For part a, HN(CH2CH2NH2)2 is tridentate not only because it has 3 N atoms with a lone pair that can form a coordinate bond, but also because it consists of all single bonds, which can rotate and keep the 3 lone pairs next to the central TM cation. For part b, all 3 oxygen atoms in CO 3 2- has l...
- Tue Dec 01, 2020 12:09 am
- Forum: Determining Molecular Shape (VSEPR)
- Topic: 2.63 in the textbook
- Replies: 1
- Views: 158
Re: 2.63 in the textbook
Hi! The structure shown on the textbook didn't draw the lone pair electrons. For part b, the oxygen has 2 lone pairs besides the 2 bonds shown in the graph, so there are 4 electron density regions in total. Therefore, the shape of electron regions is tetrahedral, and the molecular shape is bent. The...
- Thu Nov 26, 2020 5:18 am
- Forum: Lewis Structures
- Topic: HW 2E.13 (a)
- Replies: 2
- Views: 200
HW 2E.13 (a)
For the lewis structure of I 3 - , the answer says there are 2 single bonds joining the iodine atoms, and the central atom has 3 lone pairs. But what if there is 1 single bond & 1 double bond, and the central atom has 2 lone pairs? I'm not sure why this is less valid than the correct answer, sin...
- Tue Nov 24, 2020 9:39 pm
- Forum: Determining Molecular Shape (VSEPR)
- Topic: Sapling Question #18
- Replies: 2
- Views: 155
Re: Sapling Question #18
For the central C atom in [H 2 -C=C=C-H 2 ] (call it C2), it has two unhybridized p-orbitals, forming two pi bonds. Therefore, in order for the two p orbitals to co-exist and minimize electron repulsion, they must be perpendicular to each other. Then, for the two neighboring C atoms (call them C1 an...
- Tue Nov 24, 2020 9:14 pm
- Forum: Dipole Moments
- Topic: Polarity from Shape
- Replies: 12
- Views: 727
Re: Polarity from Shape
Hi! I believe all molecules with bent structure should be polar. Even if all three atoms are the same -- for example, O3 -- the molecule is still polar. The lone pair electrons and bonding electrons are arranged asymmetrically around the central atom, so the dipole moments do not cancel out.
- Mon Nov 23, 2020 10:49 pm
- Forum: Hybridization
- Topic: Sapling #18 Week7&8
- Replies: 3
- Views: 272
Re: Sapling #18 Week7&8
Hi! Because for the Carbon atom in the middle, it has 2 pi bonds formed by two 2p-orbitals. These two orbitals must be perpendicular to one another to have minimum electron repulsion (just like how px, py, and pz-orbitals are arranged in an atom). Hope it helps.
- Mon Nov 23, 2020 10:35 pm
- Forum: Wave Functions and s-, p-, d-, f- Orbitals
- Topic: Example of s-orbital wave function equation
- Replies: 2
- Views: 351
Re: Example of s-orbital wave function equation
https://chem.libretexts.org/Courses/City_College_of_San_Francisco/Chemistry_101A/Topic_E%3A_Atomic_Structure/07%3A_Electronic_Structure_of_Atoms/7.05%3A_Quantum_Mechanics_and_Atomic_Orbitals I think this is a pretty straightforward explanation of how wave functions define atomic orbitals. Hope it he...
- Mon Nov 23, 2020 10:21 pm
- Forum: Sigma & Pi Bonds
- Topic: sp3 orbitals
- Replies: 1
- Views: 204
Re: sp3 orbitals
1. Yes, the full orbital means that the lone pair will not form a bond. It will remain as a lone pair, as you see in the Lewis structure of NH3. 2. I think the hybridization model can be applied to all molecules. It's used to explain their observed structure by making several e- orbitals have equal ...
- Tue Nov 17, 2020 7:57 am
- Forum: Interionic and Intermolecular Forces (Ion-Ion, Ion-Dipole, Dipole-Dipole, Dipole-Induced Dipole, Dispersion/Induced Dipole-Induced Dipole/London Forces, Hydrogen Bonding)
- Topic: Helpful Summary of What Induced Dipole- Induced Dipole depends on
- Replies: 6
- Views: 374
Re: Helpful Summary of What Induced Dipole- Induced Dipole depends on
Charlotte Adams 2D wrote:So if there are more electrons, is the induced-dipole induced-dipole stronger and harder to break?
Thanks
Yes you're right. But induced-dipole induced-dipole interactions are all very weak compared to other interactions.
- Tue Nov 17, 2020 7:52 am
- Forum: Octet Exceptions
- Topic: Determining exceptions to the octet rule
- Replies: 2
- Views: 147
Re: Determining exceptions to the octet rule
Hi! Elements in period 3 or higher can have an expanded octet. When you draw lewis structures, if the central atom is has period >= 3 and the surrounding atoms have not yet fulfill their octet, you should consider expanding the octet of the central atom and turn some single bonds into double bonds. ...
- Tue Nov 17, 2020 7:44 am
- Forum: Ionic & Covalent Bonds
- Topic: Cation size and covalent character
- Replies: 5
- Views: 589
Re: Cation size and covalent character
Hi! Cations with higher polarizing power (which are smaller & with higher charge density) tend to form bonds with more covalent characters. This is because the cation exerts higher electrostatic attraction on the electrons surrounding the anion, causing them to delocalize and form something simi...
- Tue Nov 17, 2020 7:33 am
- Forum: Ionic & Covalent Bonds
- Topic: Liquid form of ionic compounds
- Replies: 1
- Views: 134
Re: Liquid form of ionic compounds
Hi! In the melted form (and even gaseous form), there is still attraction force between Na+ and Cl- ions, but the kinetic energy is too high to let them maintain a lattice structure like solid NaCl does. I think you are mostly right. On the microscopic level there can be Na+Cl- momentarily closely a...
- Tue Nov 17, 2020 7:16 am
- Forum: Electron Configurations for Multi-Electron Atoms
- Topic: Electron configurations for Copper
- Replies: 1
- Views: 184
Re: Electron configurations for Copper
Hi! This is because having a full 3d sub-shell makes the atom more stable with lower energy. Similarly, Cr has [Ar] 3d5 4s1 instead of [Ar] 3d4 4s2, since having half-full 3d also lowers the energy. Hope it helps!
- Wed Nov 11, 2020 11:31 pm
- Forum: Resonance Structures
- Topic: Formal Charge and Resonance
- Replies: 2
- Views: 158
Re: Formal Charge and Resonance
Hi! Not sure if I understand your question correctly. This might differ from case to case, but if the surrounding atoms are different, they will usually have different electronegativity, and the structures in which "more electronegative atoms having more negative formal charges" will be mo...
- Wed Nov 11, 2020 11:15 pm
- Forum: Interionic and Intermolecular Forces (Ion-Ion, Ion-Dipole, Dipole-Dipole, Dipole-Induced Dipole, Dispersion/Induced Dipole-Induced Dipole/London Forces, Hydrogen Bonding)
- Topic: Helpful Summary of What Induced Dipole- Induced Dipole depends on
- Replies: 6
- Views: 374
Re: Helpful Summary of What Induced Dipole- Induced Dipole depends on
That was a really nice summary!! Just to reorganize this a bit, I think the 2 major factors are Polarizability and Distance, and all others are secondary factors that influence the major factors. Factors affecting induced dipole-induced dipole interactions Ep∝(ɑ1 ɑ2)/(r^6) 1. Polarizability (∝ Elect...
- Wed Nov 11, 2020 10:59 pm
- Forum: Lewis Structures
- Topic: Sapling Week 5-6 HW Question 13
- Replies: 4
- Views: 191
Re: Sapling Week 5-6 HW Question 13
Hi! I think it's easier to explain this with a graph.
Wherever there's an H attached to N/O/F, it can form H-bond with the lone pair on O atom in H2O.
Whenever there's a lone pair on an electronegative atom (N/O/F), it can form a H-bond with the H in H2O.
Hope this helps!
Wherever there's an H attached to N/O/F, it can form H-bond with the lone pair on O atom in H2O.
Whenever there's a lone pair on an electronegative atom (N/O/F), it can form a H-bond with the H in H2O.
Hope this helps!
- Wed Nov 11, 2020 10:45 pm
- Forum: Octet Exceptions
- Topic: How far can an atom expand?
- Replies: 1
- Views: 132
Re: How far can an atom expand?
Hi! Theoretically speaking the max. # of valence electrons is the max. "capacity" of the outermost electron shell. For example, Period 3 elements can have a maximum of 18 valence electrons. Because the third electron shell can hold 18 e- (2s+6p+10d). For Period 4 elements it should be 2s+6...
- Wed Nov 11, 2020 10:36 pm
- Forum: Octet Exceptions
- Topic: 2C. 3 part b
- Replies: 2
- Views: 87
Re: 2C. 3 part b
Hi! So in the lewis structure you suggested, the sum of |formal charge| is 2, which is the same as the 3 structures in the solution manual. In this case, we need to compare the electronegativity of the atoms to determine which structure is more valid. Here, O is more electronegative than P, so O wil...
- Tue Nov 10, 2020 7:59 pm
- Forum: Dipole Moments
- Topic: Sapling Question #13
- Replies: 5
- Views: 197
Re: Sapling Question #13
Hi! I did this question and the answer should be 8. One hydrogen bond can be formed for each N-H bond, one for each N atom (since each has 1 lone pair e-), and two for the O atom (since it has 2 lone pairs of e-). According to wikipedia, a hydrogen bond is "a primarily electrostatic force of at...
- Tue Nov 10, 2020 7:40 pm
- Forum: Quantum Numbers and The H-Atom
- Topic: Quantum number ms and wave function
- Replies: 2
- Views: 142
Re: Quantum number ms and wave function
Hi! You only need the first 3 quantum numbers to specify an orbital (in which there're 2 electrons), and you'll need to include ms to specify which electron it is.
- Wed Nov 04, 2020 10:46 pm
- Forum: Ionic & Covalent Bonds
- Topic: d-block and valence electrons
- Replies: 3
- Views: 236
Re: d-block and valence electrons
Hi! Basically in the periodic table, every block that precedes a specific atom stands for an electron it has, and it is listed in a sequence as if the electron orbitals are "filled up" one by one: e.g. 4s is filled before 3d. However, valence electrons only include electrons with the large...
- Wed Nov 04, 2020 10:28 pm
- Forum: Lewis Structures
- Topic: favored structure
- Replies: 5
- Views: 145
Re: favored structure
Hi! For b and c, you can compare the electronegativity of each atom. In this case, O is more electronegative than N, and N is more electronegative than C. Therefore, O taking electrons from N (which is b) is more likely to happen than C taking electrons from N (which is c). Negative formal charges u...
- Wed Nov 04, 2020 10:18 pm
- Forum: Formal Charge and Oxidation Numbers
- Topic: lecture 11/2 question
- Replies: 2
- Views: 103
Re: lecture 11/2 question
Hi! I guess you're thinking that the electrons in d-orbital are the valence electrons. But actually the valence e- includes all electrons in the 3rd shell (n=3). So the maximum # of electrons is s2 + p6 + d10 = 18 e-. (But it doesn't mean they have to get 18 electrons. For period 3 elements it's usu...
- Wed Nov 04, 2020 10:12 pm
- Forum: Octet Exceptions
- Topic: "Octets" beyond 8
- Replies: 6
- Views: 313
Re: "Octets" beyond 8
Yes, just like Isabella said, elements in period 3 or higher can have expanded octet, and it is their stable form. Dr. Lavelle mentioned in the lecture that in these cases, the expanded octet has lower energy than octet structures, so they are more stable.
- Wed Nov 04, 2020 7:34 pm
- Forum: Octet Exceptions
- Topic: Limit on Expanding Octet
- Replies: 2
- Views: 159
Re: Limit on Expanding Octet
Hi! The maximum number of valence electrons depends on the electron orbitals the element can have. For elements with n>=3, they can have more than 8 electrons because they can have s2 + p6 + d10 = 18 electrons. For elements with n>=4, theoretically they can have s2 + p6 + d10 + f14 = 32 electrons ma...
- Wed Oct 28, 2020 12:34 am
- Forum: Photoelectric Effect
- Topic: Photoelectric Effect
- Replies: 13
- Views: 910
Re: Photoelectric Effect
Hi! If the energy of light matches the energy difference between two electron shells, then the energy will be absorbed and it will excite the electron to a higher energy level. This is the same situation as in atomic absorption spectrum. However, if the energy does not match then it will not be abso...
- Wed Oct 28, 2020 12:22 am
- Forum: SI Units, Unit Conversions
- Topic: Angstrom
- Replies: 6
- Views: 546
Re: Angstrom
Hi! I usually put the 2 units I want to convert into a fraction. For example, I know that 1m=100cm, so the fraction can be \frac{1m}{100cm} or \frac{100cm}{1m} . Because the denominator and numerator are the same, both fractions equal to 1. Then, I can multiply a value by this fraction, and cancel o...
- Wed Oct 28, 2020 12:07 am
- Forum: Properties of Light
- Topic: rydberg's constant
- Replies: 11
- Views: 993
Re: rydberg's constant
Hi! In terms of solving homework problems I have only used '3.28984 x10^15 Hz' so far. Perhaps the other value is more useful when solving other types of questions which we have not yet encounter. :)
- Tue Oct 27, 2020 11:58 pm
- Forum: Quantum Numbers and The H-Atom
- Topic: Quantum Numbers
- Replies: 3
- Views: 215
Re: Quantum Numbers
Hi! I don't think they can all be the same because the acceptable numerical values for each is different. For example, 'n' should be a natural number like 1, 2, 3, 4 ...; 'l' should be a non-negative integer from zero to (n-1); and 'ml' should be an integer from -l to l. So n and l can never be the ...
- Tue Oct 27, 2020 11:47 pm
- Forum: Quantum Numbers and The H-Atom
- Topic: Discovering Quantum Numbers
- Replies: 1
- Views: 32
Re: Discovering Quantum Numbers
Hi! I think the 3 quantum numbers are three parameters of wave function, which is the solution of Schrodinger equation. The Schrodinger Equation can determine the wave function (i.e. orbital) of an electron in an atom, and the wave function specifies the behavior of the electron wave in relation to ...
- Thu Oct 22, 2020 1:51 am
- Forum: DeBroglie Equation
- Topic: Sapling #22
- Replies: 11
- Views: 324
Re: Sapling #22
Hi! I think the main problem here is that E=hc/λ gives you the total energy of the wave, not just the kinetic energy. So you need to calculate the momentum (and thus velocity) of the electron first, and then work out Ek with 1/2mv^2. Also, the De Broglie's equation only works for particle with mass,...
- Thu Oct 22, 2020 1:35 am
- Forum: *Shrodinger Equation
- Topic: How are wave functions determined?
- Replies: 1
- Views: 75
Re: How are wave functions determined?
It's me again. I guess I kind of figured it out a little bit... Is it that we can derive the wave functions if we impose boundary conditions to them (for example, in 1 dimension, we can limit it in a length L), therefore only certain wavelengths are acceptable, and then we can determine all possible...
- Thu Oct 22, 2020 12:48 am
- Forum: *Shrodinger Equation
- Topic: How are wave functions determined?
- Replies: 1
- Views: 75
How are wave functions determined?
Hi! I know that Schrodinger Equation can be used to calculate the energy of electrons given their wave functions. But I am unsure about how the wave functions (like the s, p, d, f orbitals) were derived in the first place -- I mean, in order to determine those wave functions, we need to know the emp...
- Wed Oct 21, 2020 11:50 pm
- Forum: DeBroglie Equation
- Topic: De Broglie Wavelength vs Wavelength based on EM Spectrum
- Replies: 5
- Views: 310
Re: De Broglie Wavelength vs Wavelength based on EM Spectrum
I don't have a confident answer to this, but it might be helpful to think about "what is waving" there. For sound waves, it's the particles of the media; for EM waves it's electromagnetic fields; and for particles like electrons, it might be something else. Hope it helps!
- Wed Oct 21, 2020 11:33 pm
- Forum: Student Social/Study Group
- Topic: Hamiltonian in Schrodinger's Wave Function
- Replies: 2
- Views: 188
Re: Hamiltonian in Schrodinger's Wave Function
Hi! You can think of the Hamiltonian operator as a kind of "template" or "equation". You plug in the wave function psi and get the result (E psi) This is a screenshot of the textbook: 截屏2020-10-22 下午2.29.10.png The left hand side of the equation (H-psi) is what we get after putti...
- Wed Oct 21, 2020 11:20 pm
- Forum: Wave Functions and s-, p-, d-, f- Orbitals
- Topic: What does the wave function (not squared) mean?
- Replies: 2
- Views: 180
Re: What does the wave function (not squared) mean?
Hi! I was wondering about these questions too. What I learned from the textbook and YouTube videos is that the wave function (psi) itself doesn't really have a physical meaning, at least we haven't figured out how to interpret it. So I guess it's just a mathematical representation of "an electr...
- Fri Oct 16, 2020 2:08 am
- Forum: Properties of Light
- Topic: Are frequencies discrete?
- Replies: 1
- Views: 130
Re: Are frequencies discrete?
Hi! I believe frequency is continuous for both wave and particle model. (like when we use v=E/h to calculate frequency of photons, and the result can be a continuous range of values) However, in the wave model energy transfer is continuous (i.e. particles can absorb any amount of energy from light);...
- Mon Oct 12, 2020 11:27 pm
- Forum: Photoelectric Effect
- Topic: Post Module Assessment PhotoElectric Effect #29 & 30
- Replies: 1
- Views: 72
Re: Post Module Assessment PhotoElectric Effect #29 & 30
Hi! For Q29, the work function for sodium is 150.6 kJ per mol, so you need to divide 150.6 kJ/mol by Avogadro's constant (6.02*10^23) to get the answer (it should be 2.501x10^-19 J). And for Q30, you should also replace the threshold energy with the answer you get from Q28, since E=hv represents the...
- Mon Oct 12, 2020 11:03 pm
- Forum: Properties of Light
- Topic: Regions
- Replies: 2
- Views: 71
Re: Regions
Hi! I think the UV region refers to the light with wavelength 10-400 nm. The image below is a spectrum showing the different regions of light. They are categorized and named according to their wavelength/frequency. Hope it helps!
- Mon Oct 12, 2020 10:54 pm
- Forum: Photoelectric Effect
- Topic: What determines intensity of the light according to the photon model?
- Replies: 3
- Views: 200
Re: What determines intensity of the light according to the photon model?
Hi! In the photon model, light intensity is determined by the number of photons; and for each photon, its energy is determined by its frequency (E=hv). In the wave model, light intensity is determined by the amplitude of the wave, and energy is correlated with both amplitude and frequency. In other ...
- Mon Oct 12, 2020 10:22 pm
- Forum: Bohr Frequency Condition, H-Atom , Atomic Spectroscopy
- Topic: Rydberg's Constant
- Replies: 2
- Views: 110
Re: Rydberg's Constant
I think whether you add the negative sign or not depends on the values of n1 and n2. You just have to make sure the frequency (v) is positive. My understanding is: The Rydberg equation is essentially derived from E_n=-\frac{hR}{n^2} . The energy difference between two energy levels can be expressed ...
- Mon Oct 12, 2020 9:40 pm
- Forum: Properties of Light
- Topic: Sapling Textbook 1A.15
- Replies: 2
- Views: 113
Re: Sapling Textbook 1A.15
Hi! So after converting the wavelength into frequency using c=λv, you can plug in the frequency (v) to the Rydberg equation to determine n2. 0.112 is the value of \frac{1}{(n_2)^2} , so (n_2)^2 is equal to \frac{1}{0.112} (approximately =9). Therefore (n_2) is \sqrt\frac{1}{0...
- Mon Oct 12, 2020 9:23 pm
- Forum: Administrative Questions and Class Announcements
- Topic: CHEM 14B Co-requisite
- Replies: 1
- Views: 156
CHEM 14B Co-requisite
Hi! I'm currently enrolled in CHEM 14A. While planning my future courses, I'm wondering if CHEM 14B and MATH 31B have to be taken together? (It shows MATH 31B is the co-requisite, not pre-requisite) Is it possible to take MATH 31B first, and CHEM 14B later on?
Thank you!
Thank you!
- Sun Oct 11, 2020 12:09 am
- Forum: Properties of Light
- Topic: Origin of c=λv
- Replies: 3
- Views: 163
Re: Origin of c=λv
Hi! I'm not entirely sure of this, but I think the equation c=λv can be derived from the units. Wavelength (λ) is the distance between two peaks (measured in meter), and frequency (v) is the number of reps in each second (measured in second^-1). So if you multiply the two units you'll get m*s^-1, wh...
- Sat Oct 10, 2020 11:52 pm
- Forum: Limiting Reactant Calculations
- Topic: M9
- Replies: 3
- Views: 157
Re: M9
Hi! The reason why NaOH should be the limiting reagent, not Cu(NO3)2, is that they react in a 2:1 ratio. The chemical equation is: Cu(NO3)2 + 2 NaOH ---> Cu(OH)2 + 2NaNO3 Therefore, for 0.04 mol Cu(NO3)2, 0.08 mol NaOH is needed, but we only have 0.05 mol NaOH. So actually NaOH is the limiting reage...
- Fri Oct 09, 2020 12:51 am
- Forum: Empirical & Molecular Formulas
- Topic: L.39 Textbook question
- Replies: 3
- Views: 492
Re: L.39 Textbook question
Hi! For this question, we can first calculate the masses of the product and reactants. Given the crucible is 26.45 g, and the crucible + product are 28.35 g in total, the mass of the product (the oxide) is 28.35g-26.45g = 1.90g. And we also know that the tin sample is 1.50g. So we have: Sn (1.50g) +...
- Thu Oct 08, 2020 4:57 pm
- Forum: Molarity, Solutions, Dilutions
- Topic: Homework Problem G.25
- Replies: 1
- Views: 64
Re: Homework Problem G.25
Hi! I've posted a response under another question that asked this problem, so I'll just paste it here: --- First, we can calculate the number of molecules in the 10mL original solution: n_{initial} = c_{initial} \cdot V = 0.1 \, mol/L \cdot 10\,mL = 0.0010\,mol Then, each time the volume is doubled,...
- Wed Oct 07, 2020 12:38 am
- Forum: Empirical & Molecular Formulas
- Topic: Audio Visual Topic Video Question
- Replies: 6
- Views: 230
Re: Audio Visual Topic Video Question
Hi! we only care about molar ration when dealing with empirical formulas. The mass percent composition can be seen as the mass ratio of different elements in a sample. The ratio won't be affected by sample mass. And I want to add that when we want to find the molecular formula when given an empiric...
- Wed Oct 07, 2020 12:11 am
- Forum: Empirical & Molecular Formulas
- Topic: Audio Visual Topic Video Question
- Replies: 6
- Views: 230
Re: Audio Visual Topic Video Question
Hi! That's because, after you convert the mass of each element into the number of moles, you still need to divide each mole number by the smallest one to get the empirical formula. Only the molar ratio matters. For example, if you imagine there are 100 grams of sample, and you get 1mol C + 4mol H. T...
- Tue Oct 06, 2020 11:50 pm
- Forum: Empirical & Molecular Formulas
- Topic: M19: oxygen
- Replies: 4
- Views: 143
Re: M19: oxygen
A stimulant in coffee and tea is caffeine, a substance of molar mass 194 g/mol -1. When 0.376 g of caffeine was burned, 0.682 g of carbon dioxide, 0.174 g of water, and 0.110 g of nitrogen were formed. Determine the empirical and molecular formulas of caffeine. The unbalanced equation is: Caffeine ...
- Tue Oct 06, 2020 11:19 pm
- Forum: Accuracy, Precision, Mole, Other Definitions
- Topic: Chemical Formulas of Compounds
- Replies: 9
- Views: 430
Re: Chemical Formulas of Compounds
I don't think we need to know all the conventional names for complex molecules like fluoxetine. (But for very common ones, like glucose, it might be helpful to know.) This is just a simple way to refer to the molecule but has little to do with its molecular structure. The IUPAC name is the one that ...
- Tue Oct 06, 2020 10:37 pm
- Forum: Molarity, Solutions, Dilutions
- Topic: G.25
- Replies: 2
- Views: 79
Re: G.25
First, we can calculate the number of molecules in the 10mL original solution: n_{initial} = c_{initial} \cdot V = 0.1 \, mol/L \cdot 10\,mL = 0.0010\,mol Then, each time the volume is doubled, the concentration of the solution becomes one half, and the number of molecules in 10mL of the resultant s...
- Tue Oct 06, 2020 9:55 pm
- Forum: Limiting Reactant Calculations
- Topic: maximum amount of products
- Replies: 4
- Views: 1076
Re: maximum amount of products
Hi! The equation for that question should be 2A+1B—> 3 C, not 2A+1B—>C. The "maximum amount of product" is another way of saying the "theoretical yield". In this case, you have 1 mol A reacting with 0.5 mol B, leaving the other 0.5 mol B in excess. The question is asking for the ...